<span>N2(g) + 2 O2(g) → 2 NO2(g)
</span>
(1) N2(g) + O2(g) → 2 NO(g) Δh = +180.7 kJ
(2) 2 NO(g) + O2(g) → 2 NO2(g) Δh = −113.1 kJ
(3) 2 N2O(g) → 2 N2(g) + O2(g) Δh = −163.2 kJ
You want to rearrange the given reactions to match the reaction with the unknown enthalpy. Looking at what we're given, reaction (2) already has 2NO2 on the product side just like our unknown, so let's start there - it can stay as is.
However, it has 2NO on the reactant side - that's not in our unknown reaction, so we need to get rid of it somehow. There's 2NO in reaction (1), and it's on the product side, so it will cancel the 2NO on the reactants side of reaction (2). This means reaction (1) can stay as it is as well.
If you add these two reactions together, you'll get:
N2(g) + O2(g) + 2 NO(g) + O2(g)→ 2 NO(g) + 2 NO2(g)
N2(g) + 2O2(g) + 2 NO(g) → 2 NO(g) + 2 NO2(g)
N2(g) + 2O2(g) → 2 NO2(g)
The 2 NO cancels out and the individual O2's add together to get 2O2. This gives us the unknown reaction so we actually don't need to use reaction (3) at all to answer this question. In fact, it makes things more difficult because it contains N2O, which cannot be cancelled in any way with the reactions we're given.
To find the enthalpy of the unknown reaction, add the enthalpies of the reactions that work. Since we didn't have to modify either of the the first 2 reactions, you can add their original enthalpies as given:
+180.7 kJ + (−113.1 kJ) = +67.6 kJ
Answer:
The pressure of N₂O₄ in the reaction vessel after the reaction is 290 mmHg
Explanation:
Nitrogen gas reacts with oxygen gas to form dinitrogen tetroxide.
N₂ (g) + 2O₂ (g) → N₂O₄ (g)
Therefore since by Avogadro's law equal volumes of all gases contain equal numbers of molecules, there fore as the gases are within the same vessel, thier partial pressure is equivalent to their concentration
from the reaction, 1 mole of N₂ react with 2 moles of O₂ to produce 1 mole of N₂O₄
Thus
1 mmHg of N₂ react with 2 mmHg of O₂ to produce 1 mmHg of N₂O₄
337 mmHg N₂ ×(1 mmHg of N₂O₄/ 1 mmHg of N₂) = 337 mmHg N₂O₄
580 mmHg O₂ ×(1 mmHg of N₂O₄/ 2 mmHg of O₂) = 290 mmHg N₂O₄
As seen from the above calculation, the limting reactant is oxygen and the partial pressure of N₂O₄ = 290 mmHg
Answer:
pH = 2.25
Explanation:
pH is a measurement in chemistry defined as the -log [H₃O⁺]. Molarity [], is defined as the ratio between moles of solute (HCl) and the liters of solution
To solve this question we must find the molarity of the H₃O⁺ knowing: [HCl] = [H₃O⁺]
[HCl]:
0.0084moles / 1.500L
= 0.0056M = [HCl] = [H₃O⁺]
pH = -log [H₃O⁺] = -log [0.0056M]
<h3>pH = 2.25</h3>
Answer:
The solutions are classified according to their ability to scatter light rays.
We can't just use this property because some true solutions also contain undissolved solute.
Explanation:
Tyndall effect refers to the ability of a solution to scatter light rays. True solutions do not scatter light rays while false solutions scatter light rays.
Colloid particles are not large enough to be seen with naked eyes unlike suspensions. We should not confuse a colloid with a suspension because in a suspension, the dispersed solutes are seen with naked eye.